- ✓$2, 2-$ dimethyl propane
- B$2-$ methyl butane
- CIsobutane
- D$n-$ pentane
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Given $\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \log 4=0.6021$
$(h = 6.6 \times 10^{-34} \ J\ s)$
$(i)\,\,$on doubling the initial concentration of $A$ only, the rate of reaction is also doubled and
$(ii)$ on doubling the initial concentration of both $A$ and $B,$ there is a change by a factor of $8$ in the rate of the reaction.
The rate of this reaction is given by
$\Delta E = - 2.0 \times {10^{ - 18}}\,J\left( {\frac{1}{{n_2^2}} - \frac{1}{{n_1^2}}} \right)$
the wavelength of the light that must be absorbed to excite hydrogen electron from level $n\, = 1$ to level $n\, = 2$ will be: $(h\, = 6.625\times10^{-34}\, J\,s,\, C\, = 3\times10^8\, m\,s^{-1})$
